PET 6 Flashcards
(57 cards)
Which pair of element will combine
chemically to form an ionic compound?
A. magnesium and fluorine
B. chlorine and bromine
C. carbon and oxygen
D. hydrogen and sulfur
A. magnesium and fluorine
Carbon Dioxide is a _____
A. Element
B. Mixture
C. Compound
D. None of these choices
C. Compound
Carbon Dioxide is a compound
composed of one carbon atom and two
oxygen atoms.
The first four most abundant elements
in the earth crust are respectively.
A. 0, C,H, N
B. 0, Si, Na, Al
C. 0, Si, Al, Fe
D. 0, Si, Al, Ca
C. 0, Si, Al, Fe
You dissolve HBr in water. The name of
the solution is
A. monohydrogen bromide
B. hydrobromic acid
C. hydrogen bromic acid
D. hydrogen monobromide
B. hydrobromic acid
A colloidal state in which a liquid is
suspended in another liquid is called:
A. sol
B. Lsolution
C. emulsion
D. suspension
C. emulsion
It is a heterogeneous fluid containing
solid particles that are sufficiently large
for sedimentation.
A. Solution
B. Colloid
C. Suspension
D. None of these choices
C. Suspension
Particles will settle to the bottom in a suspended solution. Emulsions are a type of suspension, where two immiscible liquids are mixed together.
Examples of suspended solutions
include salt water, sand in water, and
muddy water.
It consist of microscopic particles
dispersed in a solvent. Its particles are
larger than the size of a molecule but
smaller than particles that can be seen
with naked eye.
A. None of these choices
B. Suspension
C. Colloid
D. Solution
C. Colloid
The Tyndall Effect is the effect of light scattering in colloidal dispersion, while showing no light in a true solution. This effect is used to determine whether a mixture is a true solution or a colloid.
Atoms with the same mass
number but different atomic number.
A. Isotones
B. Isobars
C. Isotopes
D. Isomers
B. Isobars
Isobars are atoms (nuclides) of different
chemical elements that have the same
number of nucleons. Correspondingly,
isobars differ in atomic number (or
number of protons) but have the same
mass number.
When elements A and B form a series of
compounds, the ratio of masses of B
that combine (in different compounds)
with 1 gram of A can be reduced to
small whole numbers. This is according
to what fundamental chemical law?
A. Conservation of Mass
B. Law of Multiple Proportions
C. Law of Definite Proportions
D. Law of Inertia
B. Law of Multiple Proportions
Law of multiple proportions, statement that when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole
numbers.
Quantum number is a number that
occurs in the theoretical expression for the value of some quantized property of a subatomic particle, atom, or molecule and can only have certain integral or half-integral values. Which of the following is NOT a quantum number?
A. Magnetic Quantum Number
B. Orientation Quantum Number
C. Principal Quantum Number
D. Azimuthal Quantum Number
B. Orientation Quantum Number
Orientation Quantum Number is NOT a
quantum number. The rest are all
quantum numbers. Spin Quantum
Number is the last member which is not
stated.
Protons and neutrons can be broken down further into elementary particle called
A. neutrino
B. isotopes
C. ions
D. quarks
D. quarks
This quantum number describes the
shape of orbital and is an indication of the angular momentum of the electron.It has integer values from 0 to n-1, for each individual n.
A. Spin Quantum Number
B. Principal Quantum Number
C. Azimuthal Quantum Number
D. Magnetic Quantum Number
C. Azimuthal Quantum Number
The angular momentum quantum
number is denoted [1]. It also affects the energy of the electron, but in general not as much as the principal quantum number does.
In the absence of an
electric or magnetic field around the
atom, only n and I have any effect on the
energy of the electron. The value of l
can be 0 or any positive integer up to,
but not including, the value of n for that
electron.
“When the elements are arranged in the
order of increasing atomic number,
elements with similar properties appear at periodic intervals.” This statement is known as
A. The Periodic Law
B. Law of Multiple Proportion
C. Law of Definite Proportion
D. Dalton’s Atomic Theory
A. The Periodic Law
Periodic table’s invention is generally
credited to Russian Chemist Dmitri
Mendeleev. He arranged the elements
by their increasing atomic mass.
_is a horizontal row in the
periodic table that provides the number
of the last main energy level. It is also
called as series.
A. Electron Affinity
B. Group
C. Electron Configuration
D. Period
D. Period
A period in the periodic table is one of
the horizontal rows. All of those
elements in the row have the same
number of electron shells.
It describes how easily an atom can
lose an electron.
A. Electronegativity
B. Atomic Radius
C. Electron Affinity
D. Metallic Character
D. Metallic Character
Metallic character refers to the level of
reactivity of a metal. Metals tend to lose
electrons in chemical reactions, as
indicated by their low ionization
energies. Within a compound, metal
atoms have relatively low attraction for
electrons, as indicated by their low
electronegativities.
As you go down a group, the electron
affinity generally
A. Increases
B. Decreases
C. Not changing
D. Increase then decrease
B. Decreases
The less valence electrons an atom has,
the least likely it will gain electrons.
Electron affinity decreases down the
groups and from right to left across the periods on the periodic table because the electrons are placed in a higher energy level far from the nucleus, thus a
What group in the periodic table is the
carbon group?
A. Group III A
B. Group V A
C. Group VI A
D. Group IV A
D. Group IV A
The carbon group is a periodic table
group consisting of carbon (C), silicon(Si), germanium (Ge), tin (Sn), lead (Pb).and flerovium (FI). In modern IUPAC
notation, it is called Group 14. In the
field of semiconductor physics, it is still
universally called Group IV.
Halogens belong to what group in the
periodic table?
A. Group VII A
B. Group IV A
C. Group VI A
D. Group V A
A. Group VII A
The halogens are a group in the periodic
table consisting of five chemically
related elements: fluorine (F), chlorine
(CI), bromine (Br), iodine (1), and astatine
(At).
Valency or oxidation state of hydroxide
ion (OH) is
A. -3
B. -2
C. -1
D. -4
C. -1
Hydroxide OH- has a charge of -1.
The Oxygen has an oxidation number-2 and hydrogen has the oxidation number×7.
So 0(-2)+H(+1)=0H-
A water molecule will always contain
A. 18% of oxygen and 88% of hydrogen
B. 15% of hydrogen and 85% of oxygen
C. 11% of oxygen and 89% of hydrogen
D. 11.11% of hydrogen and 88.89% of
oxygen
D. 11.11% of hydrogen and 88.89% of
oxygen
H=1.00794 g/molx2=2.01588
0=15.9994 g/molx1 =15.9994
%0=15.9994/(15.994+2.01588)×
100%=88.81%
%H= 2.01588/(15.994+2.01588)×
100%=11.19%
A chemical substance that gives up oxygen or takes on electrons from another substance.
A. Oxidizing Agent
B. Reducing Agent
C. Oxidation
D. Reduction
A. Oxidizing Agent
In chemistry, an oxidizing agent
(oxidant, oxidizer) is a substance that
has the ability to oxidize other
substances - in other words to cause
them to lose electrons. In one sense, an
oxidizing agent is a chemical species
that undergoes a chemical reaction that
removes one or more electrons from
another atom.
_is the measure of how much
of a given substance is mixed with
another substance.
A. Concentration
B. Mole fraction
C. Dilution
D. Percentage Composition
A. Concentration
In chemistry, concentration is the
abundance of a constituent divided by the total volume of a mixture. Several types of mathematical description can be distinguished: mass concentration,molar concentration, number concentration, and volume
concentration.
Compounds are mostly classified as
A. Gaseous, liquids and solids
B. Acids and bases
C. Homogenous and heterogeneous
D. Metals and non-metals
B. Acids and bases
What is electronegativity?
A. the charge on an atom in its preferred
oxidation state
B. the amount of energy released when an
electron is added to an atom
C. the amount of energy required to create
negative ions
D. the power of an atom to attract
electrons to itself
D. the power of an atom to attract
electrons to itself
